The document discusses key concepts in chemistry including: 1) Matter can be classified as having physical or chemical properties, with physical changes altering physical properties but not chemical composition and chemical changes resulting in new substances. 2) Elements are the fundamental components of matter and are represented by atomic symbols on the periodic table, while compounds are formed by chemical bonds between different elements represented by chemical formulas. 3) Most materials are mixtures that combine substances without chemical change, whereas pure substances consist of only one type of element or compound.

1. Elements of Chemistry Chapter 2

2. 2.1 Matter Has Physical and Chemical Properties

3. “ Physical properties” describe the look or feel of a substance.

9. During a “ physical change” a substance changes some physical property…

10. … but it is still the same material with the same chemical composition.

11. Chemical Property: The tendency of a substance to change into another substance.

12. Oxygen Carbon

13. Carbon dioxide

14. Carbon dioxide Oxygen Carbon

15. Animation “CO2Flask.mov”

16. Chemical Change: Any change involving a rearrangement of atoms.

17. Chemical Reaction: The process of a chemical change...

18. During a “ chemical reaction” new materials are formed by a change in the way atoms are bonded together.

19. Physical Change

20. Chemical Change

21. 2.2 Atoms Are the Fundamental Components of Elements

22. Element: Any material consisting of only one type of atom.

26. The Periodic Table

27. Atomic Symbol: One or two letters used to designate an element.

28. Carbon, C Calcium, Ca

29. Silver, Ag (Argentum) (Hydrargyrum) Mercury, Hg

30. Elemental Formula: Used to show how atoms within an element are grouped

32. N 2

33. 2 Oxygen, O

34. 3 Ozone, O

35. Oxygen Ozone

36. Oxygen Ozone Physical or chemical change?

37. 2.3 Elements Can Combine to Form Compounds

38. Compound A material in which atoms of different elements are bonded to one another.

39. Sodium chloride

40. Sodium chloride Na

41. Sodium chloride Cl

42. Ammonia

43. Ammonia N

44. Ammonia H

45. A compound is represented by its…

46. chemical formula The combination of atomic symbols of the elements of a compound

47. Ammonia

48. Ammonia, NH 3

49. Sodium chloride

50. Sodium chloride, NaCl

51. Iron oxide Fe 2 O 3 Compound Chemical Formula

52. Iron oxide Sulfuric acid Fe SO 2 O 3 H 2 4 Compound Chemical Formula

53. Iron oxide Calcium chloride Sulfuric acid Fe SO Cl 2 O 3 H Ca 2 2 4 Compound Chemical Formula

54. Compounds have properties that are uniquely different from the elements from which they are made.

55. Iron oxide Calcium chloride Sulfuric acid Fe SO Cl 2 O 3 H Ca 2 2 4 Compound Chemical Formula

56. Iron oxide Calcium chloride Sulfuric acid Fe SO Cl 2 O 3 H Ca 2 2 4 Compound Chemical Formula

57. Iron oxide Calcium chloride Sulfuric acid Fe SO Cl 2 O 3 H Ca 2 2 4 Compound Chemical Formula

58. Sodium chloride Cl Na Compound Chemical Formula

59. Sodium metal, Na

60. Chlorine gas, Cl 2

61. Reaction

62. Sodium chloride, NaCl

63. Sodium chloride, NaCl

64. Diversity! From so few elements…

65. The Periodic Table

66. Naming Compounds

67. Guideline 1 Start with the element farthest to the left in the periodic table…

68. Guideline 1 … for the element farthest to the right, add the suffix -ide

69. Example NaCl

70. The Periodic Table

71. Example NaCl Sodium ine Chlor

72. Example NaCl Sodium ide Chlor

73. Example NaCl sodium chloride

74. Guideline 2 With different possible combinations of elements…

75. Guideline 2 … use prefixes to remove any ambiguity.

76. mono- di- tri- tetra- 2 3 4 1

77. Example CO CO 2 carbon monoxide carbon dioxide

78. Example H O H O 2 dihydrogen monoxide dihydrogen dioxide 2 2

79. Example H O H O 2 dihydrogen monoxide dihydrogen dioxide 2 2 Would you drink this??

80. H O H O 2 dihydrogen monoxide dihydrogen dioxide 2 2 (water) (hydrogen peroxide)

81. Guideline 3 Common names are also sometimes used for convenience.

82. 2.4 Most Materials are Mixtures

83. Mixture A combination of two or more substances…

84. Mixture … in which each substance retains its properties.

85. Examples

86. “ salt water” Examples NaCl H O 2 +

87. “ Air” Examples N O 2 + 2

88. “ white gold” Examples Pd Au +

89. A mixture of a gas and a liquid?

90. The formation of a mixture is different from the formation of a compound.

91. The formation of a mixture The formation of a compound Chemical Change Physical Change

92. The formation of a mixture

93. The formation of a mixture

94. 2.5 Chemists Classify Matter as Pure or Impure

95. Pure Consisting of only a single element or a single compound.

96. Pure Consisting of only a single element or a single compound. “ Ideal state”

97. Impure “ not pure”

98. Impure A mixture…

99. Impure … containing two or more elements or compounds.

100. Impure … containing two or more elements or compounds. Reality

110. Impure water can be purified by… a) removing the impure water molecules.

111. Impure water can be purified by… a) removing the impure water molecules.

112. Impure water can be purified by… b) removing everything that is not water.

113. Impure water can be purified by… b) removing everything that is not water.

114. Impure water can be purified by… c) breaking down the water to its simplest components.

115. Impure water can be purified by… c) breaking down the water to its simplest components.

116. Impure water can be purified by… d) adding some disinfectant such as chlorine.

117. Impure water can be purified by… d) adding some disinfectant such as chlorine.

118. Impure water can be purified by… ?

119. 2.6 Elements Are Organized in the Periodic Table by Their Properties

133. interval

184. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 18 Groups

186. 1 2 3 4 5 6 7 Seven Periods